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Acids and Bases

Acidity and Basicity of Boric Acid

Boric acid, H3BO3, is found in some laundry detergents, antimicrobials, and pesticides. With a Ka = 5.8 x 10^-10 it is a weak acid that behaves as a monoprotic acid. Assume you titrate 20.0 mL of 0.11 M boric acid with 0.100 M NaOH. (Show work) 1. Write the equation: 2. What is the pH of the solution before titration begin

Molar Mass of Organic Compound

You have an unknown organic compound that is soluble in acetic acid. If 39.35g of this compound in 29.95ml of acetic acid (density of acetic acid is 1.0492g/mL) has a freezing point of 8.650 degrees Celsius, what is the molar mass of this organic compound? The freezing point of acetic acid is 16.60 degrees Celsius and the fre

Solutions to General Chemistry Questions

Which ion(s) is/are spectator ions in the formation of a precipitate of AgBr via combining aqueous solutions of CoBr2 and AgNO3? a. Co2+ and Ag+ b. Co2+ and NO3- c. NO3- and Br- d. NO3- e. Br- Which of the following is an exchange reaction? a. 2SO(g) + O2(g) ---> 2SO2(g) b. CaCO3(s) ---> CaO(s) + CO2(g) c. F

Calculate the pH

Calculate the pH upon diluting 2ml of 2 N HCL to a final volume of 100 ml? Calcuate the pH upon addition of 0.0075 mole of solid NaOH to 100 ml of a 0.1 M solution of acetic acid (pKa=4.7)? If equal molar amounts of Na2HPO4 and NaJpo4 are mixed in water, calcuate the resulting pH. The pKas of phosphoric acid are 2.1, 7.2,

Titration weak acid and strong base

-------------------------------------------------------------------------------- Do you feel inclined to think that titration of acid and base at equivalence point will always yield a neutral solution? Well the answer is no. Learn from the following excersie. Weak Acid - Strong Base Titration. a 50.0-mL portion of 0.200

PH Loop

I need help with the ones marked red. (See problem set in attached file).


Preparing a Buffer. The pH of blood is 7.40. Calculate the [HCO3-] / [H2CO3] ratio of a bicarbonate-carbonic acid buffer system that will effectively maintain a sample of blood at a pH of 7.40. Hint: the Henderson-Hasselbalch equation is useful for this type of problem.

pH of a Mixed Buffer Solution

A buffer solution is made of 0.100 M HOCl and 0.250 M NaOCl. What is the pH of the resulting solution when a 15.0-mL portion of 0.200 M HCl is added to 100.0 mL of the buffer?

Common Ion Effect

What is the pH of a solution that contains 0.250-M benzoic acid and 0.600-M sodium benzoate?

Ph Loop

Hello, I am trying to find out how to plug in to calculator, to solve for PH, POH and others by using what was given. Hope I provided more information this time

Calculate the concentrations of hydrogen ion and hydroxide ion

Calculate the concentrations of hydrogen ion and hydroxide ion at 25 degrees C. 1. Aniline, C6H5NH2, is used in the manufacturing of some perfumes. What are the values for a 0.035 M solution? Kb= 4.2 x 10-10 [H+]= [HO-]= 2. For a solution in which 10.0 mL of 0.100 M HCl is added to 25.0 mL of 0.100 M NaOH [

Use Reaction Equations to Describe Chemical Changes

1. A buffer was prepared from equal molar quantities of acetic acid, HC2H3O2 and sodium acetate, NaC2H3O2. Explain how the buffer keeps the pH of the solution at about the same value (a) after the addition of a few drops of a dilute HCl solution and (b) after the addition of a few drops of a dilute NaOH solution. Use reaction eq

Basic, neutral or acidic solution

1. Will the solution formed by dissolving each of the following salts in water be basic, neutral or acidic? Write the equation to show how each ion of each salt affects the PH of the solution. 1. Na3PO4 2. NH4Cl 3. CH3COONa Please show each step in detail.

Solving for pH, pOH and [H+]

Hi, I need some assistance with the following questions: 1. Processed cheese must be at a pH of 5.5 to 5.9 to prevent the growth of unwanted microorganisms. The quality control supervisor receives a report that a sample has a [OH-] of 1.2x10^-8. Find pH, pOH, [H+] of this sample. 2. How many grams of potassium hydroxid

Balancing Equations with Calcium Phosphate and Water

Please can you help me, I need to find balanced chemical equations for: a) The reaction of calcium phosphide and water to produce phosphine and calcium hydroxide; b) The oxide formed when phosphorus burns in air, dissolves in water to give a solution of phosphoric acid (H3PO4).

Using Water and Calcium Phosphide to produce phosphine

I have a selection of apparatus and materials that I could use to prepare a gas jar of dry phosphine. I have the following pieces of apparatus to use:- Wash bottle Polythene connectors Dropping funnel with rubber stopper Bent glass tube Filter funnel with paper U-tube Porcelain boat Gas jar Round bottomed flask w

pH of a Salt Solution

What is the pH of 0.50-M sodium benzoate? The benzoate ion (C7H5O2-) is the anion of benzoic acid.

Write a balanced equation

1. Write a balanced equation for the reaction of calcium phosphide with water to produce phosphine and calcium hydroxide, in a atmosphere of carbon dioxide at 0C and a pressure of 4.8mm Hg. At STP carbon dioxide has a density of 1.96g/litre, and phosphine has a density of 1.53g/litre. Liquid water is used in the reaction. 2.

Reduction Potential

Observations: 1) A reacts spontaneously with 1mol/L BNO3, 1mol/L D(NO3)2 and dilute sulfuric acid.A does not react with 1mol/L C(NO3)2. 2) B does not react with any of the 1mol/L solutions above or the dilute sulfuric acid. 3) C reacts spontaneously with dilute sulfuric acid and with 1mol/L solutions of all the other metallic

Equilibrium Equation

Could you please explain what happens when hydrogen ions are added to a mixture of barium chromate (S) and chromate ions (AQ). Would there be a precipitate and, if not, why?

Diprotic acid with ka1 and ka2

A diprotic acid, H2A, has the following ionization constants: Ka1 = 1.1E-3 and Ka2 + 2.5E10-6. In order to make up a buffer solution of pH 5.80, which combination would you choose, NaHA/H2A or Na2A/NaHa? What is pKa of the acid component? I don't understand this problem at all! I know that a diprotic substance has something i

Buffer NH3 and NH4Cl

I am really having problems with this problem: Calculate the pH of the 0.20 M NH3 and 0.15 NH4Cl buffer. What is the pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 57.5 mL of the buffer. The first part was fair enough, I got 9.35 pH, which is correct. The set up of the second part is tripping me up, I ca

Molarity, electron configuration, and concentration

Question 31 What is the molarity of a solution in which 26.0 grams of BaCl2 (molar mass = 208.2 g/mol) are dissolved in enough water to make 450.0 mL of solution? 0.278 M 0.617 M 1.00 M 3.41 M Question 32 Which element has the following electron configuration? 1s22s22p63s2 Na Mg

Calculating acid dissociation constant

A diprotic acid, H2A, has the following ionization constants: Ka1 = 1.1E-3 and Ka2 = 2.5E-6. In order to make up a buffer solution of pH 5.8, which combination would you choose, NaHA/H2A or Na2A/NaHA? I know the solution is Na2A/NaHA, but I am not sure why. What is the pKa of the acid component?

NaOH to prepare 576 ml of a solution

How much NaOH is needed to prepare 576 mL of solution with a pH 10? Is it possible to calculate concentration of a solution, OH- concentration, and H+ concentration from just a pH given (no specific base or acid)? Is the concentration of a solution the same as the concentration of [OH-] or [H+]?

Chemical quantities

I need the exact steps that are involved in solving each of these problems and how to arrive at the answers step by step so I can grasp the concept clearly. Thanks. It is very important that I see each step. 1. The gaseous hydrocarbon acetylene, C2H2, is used in welders torches because of the large amount of heat released w